salts
DESCRIPTION
Salts. Salt Solutions. The salts of weak acids can recombine with water producing basic solutions. Salt Solutions. The salts of weak bases can recombine with water producing acidic solutions. Salt Solutions. A - + H 2 O HA + OH - B + + H 2 O H + + BOH. - PowerPoint PPT PresentationTRANSCRIPT
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Salts
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Salt Solutions•The salts of weak acids
can recombine with water producing basic
solutions
![Page 3: Salts](https://reader033.vdocument.in/reader033/viewer/2022051401/5681458b550346895db2732f/html5/thumbnails/3.jpg)
Salt Solutions•The salts of weak bases
can recombine with water producing acidic
solutions
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Salt Solutions A- + H2O HA + OH-
B+ + H2O H+ + BOH
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Salt or Hydrolysis Problems
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Salt Problem•Calculate the pH of a
0.20 M solution of NaBz
• Ka = 6.4 x 10-5
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Salt Problem• Calculate the pH of a 0.10 M solution of R-
NH3Cl
• Kb = 2.5 x 10-5
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Drill:Calculate the pH of a
0.18 M solution of KC2H3O2
• Ka = 1.8 x 10-5
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Drill:Calculate the pH of a
0.16 M solution of KC7H5O2
• Ka = 6.4 x 10-5
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Salt Applications
•Salts of strong acids & weak bases make
acidic solutions
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Salt Applications
•Salts of strong bases & weak acids make
basic solutions
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Salt Applications
•Salts of strong acids & strong bases make
neutral solutions
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Predict Relative pH
•NaAc BaCl2
•KNO3 NH4Br
•KHSO4 NH4Ac
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Predict Relative pH
•KAc NaCl
•KClO2 NH4Cl
•K2SO4 NaI
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Anhydrides•Compounds without
water; that when added to water, form
other compounds
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Acid Anhydrides
•Non-metal oxides that form acids when
added to water
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Basic Anhydrides
•Metal oxides that form bases when added to water
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Predict Relative pH
•Na2O SO2
•NO2 CO2
•CaO Al2O3
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A/B eq, Buffer & Salt
Hydrolysis Problems
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Calculate the pH of 0.10 M HF.
Ka HF = 6.5 x 10-4
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7.4 g of Ca(OH)2 was added to 2.0 L of 0.075 M
H2CO3. Calculate the molarity of all ions
present in the solution.Ka1 = 4.4 x 10-7
Ka2 = 4.7 x 10-11
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Calculate the pH of 0.10 M HF in 0.20 M NaF.
Ka HF = 6.5 x 10-4
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Calculate the pH of 5.0 M KCN.
KaHCN= 5.0 x 10-10
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Calculate [H3PO4], [H2PO4-1],
[HPO4-2], [PO4
-3], [K+], [H+], & pH of 1.0 M KH2PO4 in
0.50 M K2HPO4. Ka1 = 7.5 x 10-3
Ka2 = 6.2 x 10-8
Ka3 = 4.2 x 10-13
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Calculate pH of:0.50 M MOH in
0.20 M MCl
Kb = 5.0 x 10-5
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Calculate pH of:0.20 M MCl
Kb = 5.0 x 10-5
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Review of Acid/Base descriptions and
Acid/Base, Buffer, & Salt Equilibria
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Arhenius, Bronsted-Lowry, & Lewis Acids & Bases
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Strong Acids
Strong Bases
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Acid rxns
Base rxns
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A/B Equilibrium Constants
KW, KA, KB, & pH
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Calculate pH of:
•0.025 M HNO3
•0.020 M KOH
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Calculate pH of:
•2.0 M HNO2
•Ka = 2.0 x 10-4
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Calculate pH of:•3.0 M HZ in
2.0 M KZ•Ka HZ = 3.0 x 10-5
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Calculate pH of:
•0.20 M KQ
•Ka HQ = 2.0 x 10-5
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150 mL of 0.10 M KOH was added to 100.0 mL of 0.10 M H2CO3. Calculate [H2CO3],
[HCO3-], [CO3
-2], [H+], [OH-], & pH of the solution.
Ka1 = 4.4 x 10-7
Ka2 = 4.7 x 10-11
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Calculate [H3A], [H2A-1], [HA-2], [A-3], [K+], [H+],
[OH-], & pH of 2.0 M KH2A. Ka1 = 4.0 x 10-3
Ka2 = 5.0 x 10-8
Ka3 = 2.5 x 10-13
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Calculate pH of:
•2.0 M HQ
•Ka = 2.0 x 10-6
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Calculate pH of:•6.0 M HZ in
4.0 M KZ•Ka HZ = 3.0 x 10-5
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Calculate pH of:
•0.20 M KQ
•Ka HQ = 2.0 x 10-7